Industrial Processes & Equilibrium Quiz
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5 questions, one answer each
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1. What condition must be met for a reversible reaction to reach equilibrium?
- A. It must happen in an open system
- B. It must happen in a closed system with forward and reverse rates equal
- C. The forward reaction must stop completely
- D. The temperature must be 0°C
2. In the Haber process (N₂ + 3H₂ ⇌ 2NH₃), why does increasing pressure increase the yield of ammonia?
- A. Because ammonia is a liquid at high pressure
- B. Because there are fewer gas molecules on the product side (2) than the reactant side (4)
- C. Because pressure increases the activation energy
- D. Because pressure only affects the rate, not the yield
3. What catalyst is used in the Contact process to convert SO₂ to SO₃?
- A. Iron
- B. Vanadium(V) oxide
- C. Platinum
- D. Manganese(IV) oxide
4. Why are industrial reaction conditions usually a compromise rather than the conditions that give the maximum possible yield?
- A. Because maximum yield conditions are always illegal
- B. Because the conditions must also give an acceptable rate of reaction at reasonable cost
- C. Because catalysts only work at low yield
- D. Because reversible reactions cannot reach high yields
5. The forward reaction in an industrial equilibrium is exothermic. A chemist wants to increase the equilibrium yield of product without changing pressure. What should they do to temperature, and why?
- A. Raise the temperature, because this favours the exothermic (product-forming) direction
- B. Lower the temperature, because this favours the exothermic (product-forming) direction
- C. Raise the temperature, because temperature has no effect on equilibrium position
- D. Lower the temperature, because this favours the endothermic (reverse) direction